• A state of equilibrium is reached in a closed system when the rates of the forward and reverse reactions are equal.

• The equilibrium law describes how the equilibrium constant (Kc) can be determined for a particular chemical reaction.

• The magnitude of the equilibrium constant indicates the extent of a reaction at equilibrium and is temperature dependent.

• The reaction quotient (Q) measures the relative amount of products and reactants present during a reaction at a particular point in time. Q is the equilibrium expression with non- equilibrium concentrations. The position of the equilibrium changes with changes in concentration, pressure, and temperature.

• A catalyst has no effect on the position of equilibrium or the equilibrium constant.

• The characteristics of chemical and physical systems in a state of equilibrium.

• Deduction of the equilibrium constant expression (Kc) from an equation for a homogeneous reaction.

• Determination of the relationship between different equilibrium constants (Kc) for the same reaction at the same temperature.

• Application of Le Châtelier’s principle to predict the qualitative effects of changes of temperature, pressure and concentration on the position of equilibrium and on the value of the equilibrium constant.

• Physical and chemical systems should be covered.

• Relationship between Kc values for reactions that are multiples or inverses of one another should be covered.

• Specific details of any industrial process are not required.